Home
Class 12
CHEMISTRY
The molecular formula of a commercial re...

The molecular formula of a commercial resin used for exchanging ions in water softening is `C_(8)H_(7)SO_(3)Na` (Mol.wt.206). What would be the maximum uptake of `Ca^(2+)` ions by the resin when expressed in mole per gram resin?

A

`(2)/(309)`

B

`(1)/(412)`

C

`(1)/(103)`

D

`(1)/(206)`

Text Solution

AI Generated Solution

The correct Answer is:
To determine the maximum uptake of \( \text{Ca}^{2+} \) ions by the resin \( \text{C}_8\text{H}_7\text{SO}_3\text{Na} \), we can follow these steps: ### Step 1: Understand the Reaction The resin \( \text{C}_8\text{H}_7\text{SO}_3\text{Na} \) reacts with \( \text{Ca}^{2+} \) ions to form a complex. The balanced reaction can be represented as: \[ 2 \text{C}_8\text{H}_7\text{SO}_3\text{Na} + \text{Ca}^{2+} \rightarrow \text{C}_8\text{H}_7\text{SO}_3\text{Ca} + 2 \text{Na}^+ \] From this reaction, we can see that 2 moles of the resin react with 1 mole of \( \text{Ca}^{2+} \). ### Step 2: Calculate the Moles of Resin The molecular weight of the resin \( \text{C}_8\text{H}_7\text{SO}_3\text{Na} \) is given as 206 g/mol. Therefore, the number of moles of resin in 1 gram can be calculated using the formula: \[ \text{Moles of resin} = \frac{\text{mass (g)}}{\text{molecular weight (g/mol)}} \] For 1 gram of resin: \[ \text{Moles of resin} = \frac{1 \text{ g}}{206 \text{ g/mol}} = \frac{1}{206} \text{ mol} \] ### Step 3: Determine the Moles of \( \text{Ca}^{2+} \) Ions From the stoichiometry of the reaction, we know that 2 moles of resin react with 1 mole of \( \text{Ca}^{2+} \). Therefore, 1 mole of resin will react with: \[ \text{Moles of } \text{Ca}^{2+} = \frac{1}{2} \text{ moles of resin} \] Thus, for \( \frac{1}{206} \) moles of resin: \[ \text{Moles of } \text{Ca}^{2+} = \frac{1}{206} \times \frac{1}{2} = \frac{1}{412} \text{ mol} \] ### Step 4: Express the Result The maximum uptake of \( \text{Ca}^{2+} \) ions by the resin when expressed in moles per gram of resin is: \[ \text{Maximum uptake of } \text{Ca}^{2+} = \frac{1}{412} \text{ mol/g} \] ### Final Answer The maximum uptake of \( \text{Ca}^{2+} \) ions by the resin is \( \frac{1}{412} \) moles per gram of resin. ---
Promotional Banner

Similar Questions

Explore conceptually related problems

The chemical formula of the chelating agent Versence is C_(2) H_(4) N_(2) (C_(2) H_(2) O_(2) Na) If each mol of this compound could bind 1 mol of Ca^(2+) , what would be the rating of pure Versene, expressed as mg CaCO_(3) bound per g . Of chealting agent? Ca^(2+) is expressed in terms in terms of amount of CaCO_(3) it could form. [Mw "of vesene" = 380, Mw "of" CaCO_(3) = 100 g mol^(-1)]

The amount of energy when million atoms of iodine are completely converted into I^(-) ions in the vapour state according to the equation, I_((g))+e^(-) to I^(-)_((g)) is 4.9X10^(-13) J.What would be the electron gain enthalpy of iodine in terms of KJ mol^(-1) and eV per atom? (A)295 , 3.06 (B)− 295, − 3.06 (C)439 , 5.09 (D)− 356 , − 7.08

RH_(2) (ion exchange resin) can replace Ca^(2+) ions in hard water as RH_(2)+Ca^(2+) to RCa+2H^(+) . If L of hard water after passing through RH_(2) has pH=3 then hardness in parts per million of Ca^(2+) is :

Name the phenol with molecular formula C_(7)H_(8)O which on treatment with Br_(2) water readily gives a precipitate of C_(7)H_(5)OBr_(3) .

A mixture of ferric oxide ( Fe_(2)O_(3) ) and Al is used as a solid rocket fuel which reacts to give Al_(2)O_(3) and Fe . No other reactants and products are involved . On complete reaction of 1 mole of Fe_(2)O_(3) , 200 units of energy is released. (a) Write a balance reaction representing the above change. (b) What should be the ratio of masses of Fe_(2)O_(3) and Al taken so that maximum energy per unit of fuel is released. (c) What would be energy released if 16 kg of Fe_(2)O_(3) reacts with 2.7 kg of Al.

1L of pond water contains 20mg of Ca^(2+) and 12mg of mg^(2+) ions. What is the volume of a 2N Na_2 CO_3 solution required to soften 5000L of pond water ?

An electric current is passed through electrolytic cells in series one containing Ag(NO_(3)) (eq) and other H_(2)SO_(4) (aq). What volume of O_(2) measured at 25^(@)C and 750 mm Hg pressure would be liberated form H_(2)SO_(4) if (a) one mole of Ag^(+) is deposited from AgNO_(3) solution (b) 8 xx 10^(22) ions of Ag^(+) are deposited from AgNO_(3) solution.